Incorrect Which expression shows how the cell voltage depends on [Ag+? E = [0.799 – 0.05916 log ([Ag*])] - 0.241 E = 0.799 – 0.05916 log [Ag*] - 0.241 E = 0.241 - [0.799 – 0.05916 log ([Ag*])] E = 0.241 0.799 – 0.05916 log [Ag*]
Incorrect Which expression shows how the cell voltage depends on [Ag+? E = [0.799 – 0.05916 log ([Ag*])] - 0.241 E = 0.799 – 0.05916 log [Ag*] - 0.241 E = 0.241 - [0.799 – 0.05916 log ([Ag*])] E = 0.241 0.799 – 0.05916 log [Ag*]
Principles of Instrumental Analysis
7th Edition
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
ChapterA1: Evaluation Of Analytical Data
Section: Chapter Questions
Problem A1.23QAP
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Question
please help with 3rd
![A solution prepared by mixing 22.2 mL of 0.400 M NaCl and 22.2 mL of 0.400 M KI was titrated with 0.200 M AGNO, in a
cell containing a silver indicator electrode and a saturated calomel reference electrode.
What is [Ag+] when 21.2 mL of 0.200 M AgNO, has been added? Express your answer as x, where [Ag+] is a quotient having
the form Ksp.Agl/x.
7.5 x10-16
X =
Incorrect
What is [Ag*] when 67.0 mL of 0.200 M AGNO, have been added? Express your answer as y, where [Ag*] is a quotient having
the form Ksp.Agcı/y.
1.85 x10-16
y =
Incorrect
Which expression shows how the cell voltage depends on [Ag*] ?
E = [0.799 – 0.05916 log ([Ag*])] -
- 0.241
1
E = 0.799 - 0.05916 log
- 0.241
[Ag*],
1
E = 0.241 – [0.799 – 0.05916 log ([Ag*])]
E = 0.241 - 0.799 - 0.05916 log
[Ag+]
The difference between voltages measured when 67.0 mL and 21.2 mL AGNO, have been added is 0.390 V. Using this voltage
difference and your answers to the previous questions, calculate the numerical value of the quotient Ksp.AgCı/Kp.Agl-
4.0
Ksp.AgCı/Ksp.Agl =
Incorrect](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F85d75af0-9d0f-46d1-bc88-f12255f75558%2F6fc5a6f0-8260-4fc3-9680-a5c4002cde0b%2Fonwalji_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A solution prepared by mixing 22.2 mL of 0.400 M NaCl and 22.2 mL of 0.400 M KI was titrated with 0.200 M AGNO, in a
cell containing a silver indicator electrode and a saturated calomel reference electrode.
What is [Ag+] when 21.2 mL of 0.200 M AgNO, has been added? Express your answer as x, where [Ag+] is a quotient having
the form Ksp.Agl/x.
7.5 x10-16
X =
Incorrect
What is [Ag*] when 67.0 mL of 0.200 M AGNO, have been added? Express your answer as y, where [Ag*] is a quotient having
the form Ksp.Agcı/y.
1.85 x10-16
y =
Incorrect
Which expression shows how the cell voltage depends on [Ag*] ?
E = [0.799 – 0.05916 log ([Ag*])] -
- 0.241
1
E = 0.799 - 0.05916 log
- 0.241
[Ag*],
1
E = 0.241 – [0.799 – 0.05916 log ([Ag*])]
E = 0.241 - 0.799 - 0.05916 log
[Ag+]
The difference between voltages measured when 67.0 mL and 21.2 mL AGNO, have been added is 0.390 V. Using this voltage
difference and your answers to the previous questions, calculate the numerical value of the quotient Ksp.AgCı/Kp.Agl-
4.0
Ksp.AgCı/Ksp.Agl =
Incorrect
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